Answer:
reaction rates increase because reactants move faster, collide more often, and produce more collisions with the required energy of activation.
Explanation:
<em>A</em><em>t</em><em> </em><em>h</em><em>i</em><em>g</em><em>h</em><em>e</em><em>r</em><em> </em><em>t</em><em>e</em><em>m</em><em>p</em><em>e</em><em>r</em><em>a</em><em>t</em><em>u</em><em>r</em><em>e</em><em>s</em><em>,</em><em> </em>the reactant atoms gain high kinetic energy which decreases the intermolecular forces of attraction between these atoms/molecules.
Hence the rate of collision is very high which decreases the activation energy and products are formed with in a short period of time.
Answer:
2.75 × 10⁻⁶ M/s
1.69 × 10⁻⁶ M/s
9.23 × 10⁻⁻⁷ M/s
4.43 × 10⁻⁻⁷ M/s
2.1 × 10⁻⁻⁷ M/s
Explanation:
We have the following information for the isomerization of methyl isonitrile
Time (s) [CH₃NC] (M)
0 0.0165
2000 0.0110
5000 0.00591
8000 0.00314
12000 0.00137
15000 0.00074
To calculate the average rate of reaction (r) for each interval, we need to use the following expression:
r = -Δ[CH₃NC]/Δt
Interval 0-2000 s
r = - (0.0110 M-0.0165 M)/2000 s - 0 s = 2.75 × 10⁻⁶ M/s
Interval 2000-5000 s
r = - (0.00591 M-0.0110 M)/5000 s - 2000 s = 1.69 × 10⁻⁶ M/s
Interval 5000-8000 s
r = - (0.00314 M-0.00591 M)/8000 s - 5000 s = 9.23 × 10⁻⁻⁷ M/s
Interval 8000-12000 s
r = - (0.00137 M - 0.00314 M)/12000 s - 8000 s = 4.43 × 10⁻⁻⁷ M/s
Interval 12000-15000 s
r = - (0.00074 M - 0.00137 M)/15000 s - 12000 s = 2.1 × 10⁻⁻⁷ M/s
The number of protons in an atom is equal the atomic number (= 50)
The sum of the Neutrons and Protons is the Atomic Mass (=125)
Neutrons + Protons=125
Plug in for the protons (50)
Neutrons +(50)=125
Then, once solved, we have Neutrons = 75
Assuming the atom is NOT an ion, the amount of electrons is equal to the number of protons. (protons=electrons=50=50)
Therefore:
There are 50 electrons, 50 protons, and 75 electrons.
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